Anthraquinone and quinone are produced on a large scale by the treatment of anthracene and phenol with the chromic acid. The most useful and popular source of the chromium (III) sulfate is the Cr(III) wastes that we get from the chromate oxidation of many different organic compounds. However, the other chromium III hydroxides have been reported. It results due to the partial neutralization of the hexahydrates. Most important and useful commercially is the basic chromium sulfate, which is thought to be SO 4 (CAS#3). Further heating can yield the anhydrous sulfate as well.ĭiversity of some other chromium (VI) sulfates are also known, but also have hydroxide or oxide ligands within. We can easily obtain it by heating the 18-hydrate material above 70 ☌ temperature. 15(H 2O), (CAS #1) is a green color solid that also readily dissolves inside the water.The hydrated chromium III sulfate, Cr 2(SO 4) 3 6 of the 18 water molecules in this formula are water of crystallization. We can write the formula of this compound with more descriptions such as 2(SO 4)3 18H 2O, (CAS #1) is a violet color solid that readily dissolves when we mix it with the water to give the metal aqua complex, 3+.The hydrated chromium III sulfate, Cr 2(SO 4)3 The anhydrous chromium III sulfate, Cr 2(SO 4) 3, (CAS #1) is a violet color solid that dissolves inside the water by the addition of a reducing agent, which forms chromium(II) sulfates. Image Source: PubChem The 3 chromium III sulfates well-characterized are as follows: Its chemical structure is present below in the form of a picture, in the common illustrations we basically use for the organic molecules. The percentage by weight of any atom or group of atoms in a compound can be computed by dividing the total weight of the atom (or group of atoms) in the formula by the formula weight and multiplying by 100.1.4 Solved Example for You: Chromium III Sulfate Formula and Structure If the formula used in calculating molar mass is the molecular formula, the formula weight computed is the molecular weight. The formula weight is simply the weight in atomic mass units of all the atoms in a given formula. When calculating molecular weight of a chemical compound, it tells us how many grams are in one mole of that substance. Using the chemical formula of the compound and the periodic table of elements, we can add up the atomic weights and calculate molecular weight of the substance.įinding molar mass starts with units of grams per mole (g/mol). For bulk stoichiometric calculations, we are usually determining molar mass, which may also be called standard atomic weight or average atomic mass. This is not the same as molecular mass, which is the mass of a single molecule of well-defined isotopes. This is how to calculate molar mass (average molecular weight), which is based on isotropically weighted averages. The atomic weights used on this site come from NIST, the National Institute of Standards and Technology. This site explains how to find molar mass. The reason is that the molar mass of the substance affects the conversion. To complete this calculation, you have to know what substance you are trying to convert. These relative weights computed from the chemical equation are sometimes called equation weights.Ī common request on this site is to convert grams to moles. In chemistry, the formula weight is a quantity computed by multiplying the atomic weight (in atomic mass units) of each element in a chemical formula by the number of atoms of that element present in the formula, then adding all of these products together.įormula weights are especially useful in determining the relative weights of reagents and products in a chemical reaction.
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